The reaction between ethanol C2H5OH and water H2O is a chemical reaction and is exothermic.
Option A is correct.
<h3>What is a chemical reaction?</h3>
A chemical reaction is a rearrangement between the ions and molecules of a substance. For a chemical reaction to take place, bonds are broken in the reactants and new bonds are formed in the products.
The chemical reaction between ethanol and water is;
- This reaction is exothermic because molecules move from a higher state of energy to lower states.
- The resulting volume is also lesser than the initial volumes of the reactants according to Henry's Law, showing that heat is given off to the walls of the container.
Therefore, we can conclude that A chemical reaction occurs, as evidenced by the volume of the resultant mixture being less than the total volume of the initial components.
Learn more about the chemical reaction here:
brainly.com/question/26018275
Answer:
stars are mater, lines are not
Explanation:
The answer is 3%.
There's 100 J for growth from a total of 3000J ingested. To find out what percentage of J are used for growth, you need to figure out how much 100 of 3000 is. To do this, you divide 100/3000=0.0333. To turn it into a percent, you have to times it by 100 again, so 0.0333 x 100 = 3.33.
Briefly explain one example of targets of repression in American society, stemming from American involvement in World War I.
Answer:
A. LaborUnions, Legislation on labor and work reform
Explanation:
Unionized labor often improves the wages corporations pay across the committee to their workers. ... Collective agreement arrangements generate significant advantages for workers who may not be interested in raising production because they earn a higher salary.
The Labor Reform Act of 1977 was a recommended United States Act of Congress on US labor legislation that never came into dominance. It would have modified the labor law to bring it in line with modern advancements and global standards, by eliminating obstacles from employers to unions structure in the workplace.
